Course Review – Unit 1 Chemistry
Science 10
Science 10- Course Review
Unit 1-Chemistry - KEY
Name _________________________________
Date _____________________________
Date due __________________________
The Science 10 Chemistry Unit covers:
 Chapter 8-Elements and the Periodic Table
 Chapter 9-Chemical Formulas and Compounds
 Chapter 10-Chemical Reactions
You can also consult the “Chemistry Outline” which shows all of the activities (Worksheets and
Labs) If you don’t have one or if you want to view or print any of the activities, go to the Science
10 Web page at http://sd67.bc.ca/teachers/dcolgur and click “Science 10”
1.
2.
When zinc metal is placed in a solution of hydrochloric acid, it fizzes producing hydrogen
gas and zinc chloride.
a)
The reactants are
________zinc & hydrochloric acid_______________
b)
The products are
_____ hydrogen gas and zinc chloride _____________
c)
A word equation is:
_ zinc + hydrochloric acid  hydrogen + zinc chloride
In the following table, name the 3 major particles in the atom, state where they are located
(in the nucleus or on the outside), state their relative mass compared to a proton (assume
mass of a proton = 1) and their charge.
Particle
Location
Mass (Proton = 1)
Charge
Proton
nucleus
1
+
Neutron
nucleus
1
0
Electron
outside
1/1837
-
Course Review – Unit 1 Chemistry
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Course Review – Unit 1 Chemistry
Science 10
List the four main points in John Dalton’s atomic theory.
3.
1. All matter is made up of atoms
2. Each element has its own kind of atom. Atoms of the same element have the same
mass. Atoms of different elements have different masses.
3. Compounds are created when atoms of different elements link to form “compound
atoms”
4. Atoms cannot be created or destroyed
4.
Isotopes of an element are two different forms which have the same number of _protons
and _electrons____, but with different numbers of neutrons_____.
5.
The atomic __mass___ of an element is the average mass of the isotopes which occur in
nature.
6.
In a neutral atom, the number of electrons is always equal to the number of
___protons_____ or the ____atomic_________ number.
7.
According to the model of the atom proposed by Neils Bohr, electrons move around the
atom in _____orbits__________ or _______shells_____. When one orbit is
filled, the electrons start filling the __next higher___ orbit.
8.
The first orbit holds
_____2___ electrons.
The second orbit holds _____8_____ electrons.
The third orbit holds
9.
____8______ electrons.
Give the total number of electrons and the number of electrons in each orbit for each of the
following elements:
Element
Total # of Electrons Electrons Electrons Electrons
electrons in Level 1 in Level 2 in Level 3 in Level 4
Aluminum (Al)
13
2
8
3
7
2
5
Nitrogen (N)
20
2
8
8
Calcium (Ca)
2
3
2
1
Lithium (Li)
18
2
8
8
Argon (Ar)
Course Review – Unit 1 Chemistry
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Course Review – Unit 1 Chemistry
Science 10
10. Draw the Bohr models for neutral atoms of each of the following elements.
a)
oxygen (8 e-)
O
b)
chlorine (17 e-)
Cl
c)
phosphorus (15 e-)
P
d)
magnesium (12 e-)
Mg
11. According to Bohr, when a sample of an element is energized by heat or electricity, the
electrons jump to higher orbits. When they jump back down
to lower orbits, they give off the energy in the form of light
The amount of energy released in each jump corresponds to a certain wavelength (colour)
of light. The pattern of different colours of light given off is called the spectrum
for that element and can be seen through a device called a spectroscope. Because every
element has its own set of electrons and orbits, the spectrum given off by each element will
be different from that of any other element. What can this be used for? identification
12. What are some practical uses for pure oxygen? Welding (oxy-acetylene) First aid for
drowning, heart attack etc. victims. Rockets (eg space shuttle)
What is the main danger of pure oxygen? Makes flammable materials burn faster or
explosively
Course Review – Unit 1 Chemistry
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Course Review – Unit 1 Chemistry
Science 10
13. Phosphorus is stored in ___water__________. Suggest why? It is highly flammable and
undergoes spontaneous combustion.
14. Why is phosphorus considered a dangerous element? _can cause severe burns and cause
fires__
Suggest a practical use for elemental phosphorus
_flares, match heads_________
15. In order to have the same number of electrons as the noble gas neon, sodium
would have to lose 1 electron.
Sodium is stored in _oil or kerosene__. Suggest why? It reacts with oxygen in the air
and violently with water to produce hydrogen gas.
16. Is potassium more or less reactive than sodium __more______. Find rubidium on your
periodic table. Do you think rubidium would be more or less reactive
than potassium? __even more reactive________.
17. Name iodine Symbol _I_ Atomic number _53__ # of electrons _53__
In order to have the same number of electrons as the noble gas xenon, iodine
would have to gain 1 electron. Is iodine a metal or non-metal? non-metal
18. Classify each of the following elements as an alkali metal, alkaline earth, halogen, noble
gas or transition metal:
Element
Fe
Br
K
Kr
Ba
F
Pt
Li
Ne
Ra
Course Review – Unit 1 Chemistry
Family
Transition metal
Halogen
Alkali metal
Noble gas
Alkaline earth
Halogen
Transition metal
Alkali metal
Noble gas
Alkaline earth
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Science 10
Course Review – Unit 1 Chemistry
19. Mendeleev arranged the elements in order of atomic mass
and also put them in groups based on similar chemical and physical properties_.
20. What did Mendeleev do when he came to a space where no known element would fit?
He left it blank, predicted properties for it using nearby elements, predicted that the
element would be found.
21. Vertical columns of the Periodic Table are known as Groups or Chemical Families.
22. Elements are no longer listed in order of atomic mass, but in order of atomic number.
23. What is similar about elements in the same family? Similar chemical & physical
properties
24. What is the main use of helium?Lighter than air balloons, welding, lasers
25. What are some uses of argon?Fills incandescent light bulbs, also used in welding
26. Where is neon used?Mainly neon signs – used in some lasers
27. Where are krypton and xenon used? Strobe lights, high intensity flash bulbs
28. Why is the element radon considered dangerous even though it is not chemically reactive?
It is radioactive and could cause lung cancer
29. What would alkali metal atoms need to do in order to end up with the same stable electron
arrangements as the noble gases? Lose 1 electron
30. What can be said about the chemical reactivity of the alkali metals?highly reactive with
O2 , H2O , halogens and other elements
31. When alkali metals are put into water, what happens? They react to form hydrogen gas
and the alkali metal hydroxide. (eg. 2Na + 2H2O  H2 + 2NaOH )
32. The outer orbits of halogen atoms each have 7 electrons. This is one
(more/less) less than the nearest noble gas atom.
33. In order to achieve the stable arrangement of noble gas atoms, each halogen atom would
have to gain 1 electron.
34. Are the halogens metals or non-metals? Non-metals
Course Review – Unit 1 Chemistry
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Course Review – Unit 1 Chemistry
Science 10
35. What can be said about the chemical reactivity of the halogens? very reactive
36. Why, other than reactivity, are halogens considered dangerous to work with? very toxic
37. Fill in the following table:
Indicators in Known Acids and Bases
Indicator
Colour in Acid
Colourless
Colour in Base
Pink
Yellow
Blue
Red Litmus
Red
Blue
Blue Litmus
Red
Blue
Phenolphthalein
Bromthymol Blue
38. Are the pH’s of Acid Solutions < 7, >7 or = 7?
<7
Are the pH’s of Base Solutions < 7, >7 or = 7? >7
39. The more acidic a solution is, the (lower/higher) the pH? lower
40. The more basic a solution is, the (lower/higher) the pH? higher
41. A solution with a pH = 7 is said to be neutral
42. An acid HCl is mixed with a base KOH. Predict the chemical formulas for the two
products of this reaction. H2O and KCl. This
type of reaction of an acid reacting with a base is called neutralization
43. List 4 properties (characteristics) all acids have in common:
taste sour
turn litmus red, bromthymol blue-yellow and colourless in phenolphthalein
conduct electricity in solution
neutralize bases
react with active metals to produce hydrogen gas
Course Review – Unit 1 Chemistry
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Course Review – Unit 1 Chemistry
44. List 4 properties (characteristics) all bases have in common:
taste bitter
feel slippery
turns litmus blue, bromthymol blue-blue and pink in phenolphthalein
neutralize acid
45. What is the name of the acid found in sour milk? Lactic acid
46. What is the name of the acid found in pop? Carbonic acid
47. What is the name of the acid found in lemons and grapefruit? Citric acid
48. What is the name of the acid found in your stomach? Hydrochloric acid
49. What is the name of the acid found in car batteries? Sulphuric acid
50. What is the name of the acid found in rhubarb? Oxalic acid
51. What is the name of the acid found in apples? Malic acid
52. What is the name of the acid found in vinegar? Acetic acid
53. What is the name of the base found in oven cleaner? Sodium hydroxide
54. Acid spills can sometimes be neutralized by which common compound?
Sodium hydrogen carbonate (sodium bicarbonate) (baking soda)
55. Base spills can sometimes be neutralized by which common compound? vinegar
56. What is the chemical formula for common table salt? NaCl
57. What is the chemical name for baking soda? Sodium hydrogen carbonate
(sodium bicarbonate)
58. What is the chemical formula for baking soda? NaHCO3
59. Which family of elements has just enough electrons in their highest orbits to
completely fill them up? noble gases
Course Review – Unit 1 Chemistry
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Course Review – Unit 1 Chemistry
Science 10
60. If Lithium is combined with Fluorine, the Lithium atom will give an
electron to the Fluorine atom.
61. When Fluorine has gained an electron, it now has 9 protons (remember, it doesn’t lose
any protons),
and 10 electrons. Because protons are positive (+) and electrons are
negative (-), the charge left over is -1. The Fluorine is no longer a neutral atom, but
is a charged atom, which is called a Fluoride ion.
62. Because the lithium ion (Li+) and the fluoride ion (F-) have opposite charges, they
attract each other. This attraction forms an ion
bond.
ic
63. Generally, combining capacity means the number of electrons an atom
needs to lose or gain in order to have the same number of electrons as a noble gas
64. The combining capacity of chromium (III) is 3+
The combining capacity of manganese (IV) is 4+
The combining capacity of iron (II) is .…....... 2+
The combining capacity of copper (I) is ….... + (1)
65. Use the Periodic Table and the method shown to you by the teacher to write the correct
formulas for the following ionic compounds.
a)
magnesium iodide ...........
MgI2
b)
aluminum fluoride ........
AlF3
c)
calcium sulphide ........
CaS
Course Review – Unit 1 Chemistry
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Course Review – Unit 1 Chemistry
Science 10
d)
rubidium oxide ........
Rb2O
e)
sodium phosphide ........
Na3P
f)
iron (III) sulphate ........
Fe2(SO4)3
g)
manganese (IV) oxide ........
MnO2
h)
copper (II) phosphate ........
Cu3(PO4)2
i)
calcium nitrate ........
Ca(NO3)2
j)
ammonium chloride ........
NH4Cl
k)
lithium oxalate ........
Li2C2O4
l)
nickel (III) carbonate ........
Ni2(CO3)3
m) copper (I) permanganate ........
CuMnO4
n)
ammonium sulphate ........
(NH4)2SO4
Course Review – Unit 1 Chemistry
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Course Review – Unit 1 Chemistry
Science 10
66. Compounds with only two elements are called binary compounds.
67. In a binary compound, the non-metal changes it’s name so it ends in the letters IDE
68. In a compound containing a polyatomic ion, the name of the polyatomic ion
(always/sometimes/never) never changes.
69. Write the correct names for the following ionic compounds Spelling counts!
a)
Na3PO4 .....................
sodium phosphate
b)
K2S .........................
potassium sulphide
c)
Rb2SO3 .....................
rubidium sulphite
d)
(NH4)2CO3 ..................... ammonium carbonate
e)
Ba(OH)2 ....................
barium hydroxide
f)
MgSO4 .....................
magnesium sulphate
g)
Cs2HPO4 ......................
cesium monohydrogen phosphate
h)
NaHCO3 .....................
sodium bicarbonate (hydrogen carbonate)
i)
AgNO3 .......................
silver nitrate
j)
Na3As .......................
sodium arsenide
k)
NH4NO3 .......................
ammonium nitrate
l)
Ag2Cr2O7 .......................
silver dichromate
70. In an ionic compound, electrons are transferred from one atom
to the other. The element that lost electron(s) becomes a (+/-) + ion and the
element than gains electron(s) becomes a (+/-) - ion. The two oppositely charged
ions now (attract/repel) attract each other.
Course Review – Unit 1 Chemistry
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Course Review – Unit 1 Chemistry
Science 10
71. In a covalent compound, one atom shares electrons with another atom.
72. Show the Bohr model for a molecule of F2.
F
F
73. Give the formulas for molecules of the seven diatomic elements. The first one is H2.
H2 O2 N2 F2 Cl2 Br2 I2 (At2)
74. Draw the Bohr model for a molecule of ammonia (NH3).
H
N
H
H
75. Write the correct formulas for the following covalent compounds:
a)
nitrogen trioxide
NO3
b)
silicon tetrafluoride SiF4
c)
nitrogen monoxide
d)
selenium hexafluoride SeF6
e)
phosphorus pentachloride PCl5
f)
sulphur dioxide SO2
g)
dinitrogen tetroxide N2O4
NO
76. Write the correct names for the following covalent compounds:
a)
PF5 ..............
phosphorus pentafluoride
b)
SO3 ..............
sulphur trioxide
c)
ClF6 .............. chlorine hexafluoride
Course Review – Unit 1 Chemistry
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Course Review – Unit 1 Chemistry
Science 10
d)
SeO2..............
selenium dioxide
e)
N2O .............. dinitrogen monoxide
f)
N2Cl4 ............ dinitrogen tetrachloride
77. What is meant by a physical change? A change in which the chemical composition of the
material does not change
Give 3 examples of physical changes:
melting, freezing, boiling, condensation, sublimation, dissolving, mixing
cutting, hammering, stretching, etc. etc.
78. What is meant by a chemical change? A change in which existing substance(s) is (are)
used up and (a) new substance(s) is (are) formed.
Give 3 examples of chemical changes:
combustion, photosynthesis, decomposition , cellular respiration, synthesis,
single replacement, double replacement, neutralization, explosion etc. etc.
79. Balance the following equations by putting the proper coefficients wherever they are
needed.
a)
2Sr
+
O2

b)
2Al
+
6H2O

c)
4Al
d)
C5H12
e)
2Na
f)
2NaClO3

g)
Ca(NO3)2
+
+
3O2
+

+
2Al(OH)3
5CO2
+
H2
+
+
3O2

2H2O
2NaCl
(NH4)2SO4
Course Review – Unit 1 Chemistry
+
3H2
2Al2O3

8O2
2SrO

6H2O
2NaOH
CaSO4
+
2NH4NO3
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Course Review – Unit 1 Chemistry
Science 10
+
 2CO2
h)
C2H5OH
3O2
i)
2Al(NO3)3
j)
2NH3
k)
2C6H6
l)
S8
m)
3HNO3
n)
Br2
+
CaCl2

o)
3Mg
+
2AlCl3

+

+
+
3H2O
Al2(CrO4)3
+
6KNO3
+ 3H2

15O2
8O2
+

3K2CrO4
N2
+

+ 6H2O
8SO2
Fe(OH)3
Course Review – Unit 1 Chemistry
12CO2

3H2O
CaBr2
3MgCl2
+
+
Fe(NO3)3
Cl2 (already balanced)
+
2Al
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